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shusha [124]
3 years ago
11

Complete combustion of a sample of a hydrocarbon on excess oxygen produces equimolar quantities of carbon dioxide and water. Whi

ch of the following could be the molecular formula of the compound?
A. C2H2
B.C2H6
C.C4H8
D.C6H6
Chemistry
1 answer:
Bond [772]3 years ago
6 0
<span>C. C4H8 Given that the number of moles of CO2 and H2O produced from the combustion are equal, that means for every carbon atom, there are 2 hydrogen atoms because CO2 has only 1 carbon atom and H2O has 2 hydrogen atoms. So let's look at the available choices and see which one is correct. A. C2H2 This is a 1 to 1 ratio of carbon to hydrogen. Wrong answer. B. C2H6 This is a 1 to 3 ratio of carbon to hydrogen. Wrong answer. C. C4H8 This is a 1 to 2 ratio of carbon to hydrogen. Correct answer. D. C6H6 This is a 1 to 1 ratio of carbon to hydrogen. Wrong answer.</span>
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Consider the following intermediate chemical equations.
QveST [7]

Answer: 250 kJ

Explanation: According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to Hess’s law, the chemical equation can be treated as algebraic expressions and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

P_4(s)+6Cl_2\rightarrow 4PCl_3  \Delta H_1=-2439kJ (1)

4PCl_5(g)\rightarrow P_4(s)+10Cl_2(g)  \Delta H_2=3438kJ (2)

Net chemical equation:

PCl_5(g)\rightarrow PCl_3(g)+Cl_2(g)  \Delta H=? (3)

Adding 1 and 2 we get,

4PCl_5(g)\rightarrow 4PCl_3(g)+4Cl_2 \Delta H_3=\Delta H_1+\Delta H_2=-2439+3438=1000kJ   (4)

Now dividing equation (4) by 4, we get

PCl_5(g)\rightarrow PCl_3(g)+Cl_2

\Delta H=\frac{\Delta H_3}{4}=\frac{1000kJ}{4}=250kJ   (4)

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Classify the following compounds as binary ionic, ternary ionic, or molecular.
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Explanation:

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